Alternative Solvents for Catalysis and Organic Reactions

Total Page:16

File Type:pdf, Size:1020Kb

Alternative Solvents for Catalysis and Organic Reactions ALTERNATIVE SOLVENTS FOR CATALYSIS AND ORGANIC REACTIONS A Thesis Presented to The Academic Faculty By Vittoria Madonna Blasucci In Partial Fulfillment of the Requirements for the Degree Doctor of Philosophy in Chemical & Biomolecular Engineering Georgia Institute of Technology December 2009 ALTERNATIVE SOLVENTS FOR CATALYSIS AND ORGANIC REACTIONS Dr. Charles A. Eckert, Advisor School of Chemical & Biomolecular Engineering Georgia Institute of Technology Dr. Charles L. Liotta, Co-Advisor School of Chemistry & Biochemistry Georgia Institute of Technology Dr. William Koros School of Chemical & Biomolecular Engineering Georgia Institute of Technology Dr. Christopher Jones School of Chemical & Biomolecular Engineering Georgia Institute of Technology Dr. Amyn Teja School of Chemical & Biomolecular Engineering Georgia Institute of Technology Date Approved: September 30th 2009 For my Mom and Dad- Without them I would have never made it through ACKNOWLEDGEMENTS First, I would like to acknowledge my advisor, Prof. Charles Eckert. Under his guidance, I was given the freedom to take my research into the areas that interest me the most. Not only is he a valuable information source, but he is also an excellent mentor. In addition, I thank my co-advisor, Prof. Charles Liotta. It has been my pleasure to work with someone who truly loves what they do and refreshing to see somebody who enjoys science so much. Due to these two professors, my time at Georgia Tech has been excellent. I greatly appreciate the time and advice of my committee members: Professors Amyn Teja, Bill Koros, and Chris Jones. Thank you for reading through and editing this document! I would also like to acknowledge Dr. Gelbaum for his assistance with several NMR experiments and a former co-worker from Chevron, Robert Shong, who ran oil analysis experiments. I am especially grateful to the past and present Eckert/Liotta research group members. They have been enjoyable to work with and have become life-long friends. I specifically want to acknowledge two colleagues who greatly contributed to my research: Jason Hallett and Megan Donaldson. I appreciate the laboratory assistance from Georgina Schaefer, an undergraduate researcher. I wouldn’t have been able to make it through my PhD without the help of my friends and family. My mother and father have supported me throughout my academic career. Even though it took longer than they expected, I finally made my dream come true! Thank you to my sister, Dr. Madelena Blasucci, who has always been there. The iv strength of my uncle, Michael Blasucci (1959-2009), taught me to fight through even the worst of situations. Special thanks to Krystle Chavez for her friendship and to Zainul Husain for his friendship and entertainment during long lab days. Lastly, but most importantly, I would like to thank God for always keeping an eye over me and blessing me each day. v TABLE OF CONTENTS ACKNOWLEDGEMENTS ............................................................................................... iv LIST OF TABLES ............................................................................................................. xi LIST OF FIGURES .......................................................................................................... xii LIST OF SCHEMES........................................................................................................ xvi NOMENCLATURE ....................................................................................................... xvii SUMMARY ...................................................................................................................... xx CHAPTER 1. INTRODUCTION .......................................................................................1 1.1. References ........................................................................................................... 4 CHAPTER 2. ONE-COMPONENT, SWITCHABLE IONIC LIQUIDS DERIVED FROM SILYLATED AMINES ...........................................................................................5 2.1. Introduction ......................................................................................................... 5 2.2. Materials ............................................................................................................. 7 2.3. Experimental Methods ........................................................................................ 8 2.3.1 Ionic Liquid Formation ............................................................................... 8 2.3.2 Hydrosilylation Reactions ........................................................................... 9 2.3.3 Viscosity Experiments ................................................................................ 9 2.3.4 Nile Red Polarity Tests ............................................................................. 10 2.3.5 Differential Scanning Calorimetry (DSC)/Thermal Gravimetric Analysis (TGA) …………………………………………………………………………... 10 2.3.6 Crude Oil Purification Proof of Principle Recycles .................................. 10 2.3.7 Carbon Capture Capacity .......................................................................... 11 2.3.8 Stability Tests............................................................................................ 12 vi 2.3.9 Scale-up Simulations ................................................................................ 12 2.4. Results ............................................................................................................... 13 2.4.1 Siloxylated Amines ................................................................................... 13 2.4.2 Application to Hydrocarbon Extraction from Crude Oil .......................... 27 2.4.3 Silylated Amine Synthesis and Characterization ...................................... 32 2.4.4 Amine Stability ......................................................................................... 43 2.4.5 Application to Carbon Capture from Post-Combustion Flue Gas Streams ………………………………………………………………………….. 46 2.4.6 Intramolecular Interaction: Siloxylated Amine Precursors....................... 49 2.5. Conclusions ....................................................................................................... 54 2.6. References ......................................................................................................... 55 CHAPTER 3. HOMOGENEOUS CATALYSIS COUPLED WITH BENIGN SEPARATION IN POLYETHYLENE GLYCOL-ORGANIC-TUNABLE SOLVENT SYSTEMS …………………………………………………………………………... 58 3.1. Introduction ....................................................................................................... 58 3.2. Materials ........................................................................................................... 66 3.3. Experimental Methods ...................................................................................... 67 3.3.1 Reaction of 2-chloro-p-xylene and potassium hydroxide to produce 2,5-di- methylphenol in POTS .............................................................................................. 67 3.3.2 Reaction of 1-bromo-3,5-di-tert-butylbenzene with potassium hydroxide to produce 3,5-di-tert-butylphenol in POTS ............................................................. 68 3.3.3 Reaction of 2-chloro-p-xylene with basic salts to produce 1,1’-oxybis[2,5- dimethyl]benzene ...................................................................................................... 69 3.3.4 Reaction of 2-chloro-p-xylene with phenol and basic salts to produce 2,5- dimethyl-1-phenoxybenzene ..................................................................................... 70 3.3.5 Reaction of 1-bromo-3,5-di-methylbenzene and o-cresol with potassium hydroxide to produce o-tolyl-3,5-xylyl ether in POTS ............................................. 70 vii 3.3.6 Separation of 3,5-di-tert-butylphenol using POTS ................................... 71 3.3.7 Separation of o-tolyl-3,5-xylyl ether using POTS .................................... 72 3.3.8 Separation of PdL12 using POTS .............................................................. 72 3.3.9 Sweeping Carbon Dioxide Extraction of 2,4-di-methylphenol and o-tolyl- 3,5-xylyl ether from PEG 400 ................................................................................... 74 3.4. Results ............................................................................................................... 74 3.4.1 C-O coupling to produce phenols ............................................................. 74 3.4.2 C-O coupling to produce aromatic ethers ................................................. 82 3.4.3 Sweeping CO2 ........................................................................................... 87 3.4.4 Partitioning ................................................................................................ 88 3.5. Conclusions ....................................................................................................... 94 3.6. References ......................................................................................................... 95 CHAPTER 4. FUNCTIONALIZATION OF ETHYLENIC POLYMERS WITH SILANES …………………………………………………………………………. 98 4.1. Introduction ....................................................................................................... 98 4.2. Experimental Methods .................................................................................... 102 4.2.1 Materials ................................................................................................
Recommended publications
  • Cyanide Remediation: Current and Past Technologies C.A
    CYANIDE REMEDIATION: CURRENT AND PAST TECHNOLOGIES C.A. Young§ and T.S. Jordan, Department of Metallurgical Engineering, Montana Tech, Butte, MT 59701 ABSTRACT Cyanide (CN-) is a toxic species that is found predominantly in industrial effluents generated by metallurgical operations. Cyanide's strong affinity for metals makes it favorable as an agent for metal finishing and treatment and as a lixivant for metal leaching, particularly gold. These technologies are environmentally sound but require safeguards to prevent accidental spills from contaminating soils as well as surface and ground waters. Various methods of cyanide remediation by separation and oxidation are therefore reviewed. Reaction mechanisms are given throughout. The methods are compared in regard to their effectiveness in treating various cyanide species: free cyanide, thiocyanate, weak-acid dissociables and strong-acid dissociables. KEY WORDS cyanide, metal-cyanide complex, thiocyanate, oxidation, separation INTRODUCTION ent on the transport of these heavy metals through their tissues, cyanide is very toxic. Waste waters from industrial operations The mean lethal dose to the human adult is transport many chemicals that have ad- between 50 and 200 mg [2]. U.S. EPA verse effects on the environment. Various standards for drinking and aquatic-biota chemicals leach heavy metals which would waters regarding total cyanide are 200 and otherwise remain immobile. The chemicals 50 ppb, respectively, where total cyanide and heavy metals may be toxic and thus refers to free and metal-complexed cya- cause aquatic and land biota to sicken or nides [3]. According to RCRA, all cyanide species are considered to be acute haz- die. Most waste-water processing tech- ardous materials and have therefore been nologies that are currently available or are designated as P-Class hazardous wastes being developed emphasize the removal of when being disposed of.
    [Show full text]
  • Acids and Bases
    Name Date Class CHAPTER 14 REVIEW Acids and Bases SECTION 1 SHORT ANSWER Answer the following questions in the space provided. 1. Name the following compounds as acids: sulfuric acid a. H2SO4 sulfurous acid b. H2SO3 hydrosulfuric acid c. H2S perchloric acid d. HClO4 hydrocyanic acid e. hydrogen cyanide 2. H2S Which (if any) of the acids mentioned in item 1 are binary acids? 3. Write formulas for the following acids: HNO2 a. nitrous acid HBr b. hydrobromic acid H3PO4 c. phosphoric acid CH3COOH d. acetic acid HClO e. hypochlorous acid 4. Calcium selenate has the formula CaSeO4. H2SeO4 a. What is the formula for selenic acid? H2SeO3 b. What is the formula for selenous acid? 5. Use an activity series to identify two metals that will not generate hydrogen gas when treated with an acid. Choose from Cu, Ag, Au, Pt, Pd, or Hg. 6. Write balanced chemical equations for the following reactions of acids and bases: a. aluminum metal with dilute nitric acid ϩ → ϩ 2Al(s) 6HNO3(aq) 2Al(NO3)3(aq) 3H2(g) b. calcium hydroxide solution with acetic acid ϩ → ϩ Ca(OH)2(aq) 2CH3COOH(aq) Ca(CH3COO)2(aq) 2H2O(l ) MODERN CHEMISTRY ACIDS AND BASES 117 Copyright © by Holt, Rinehart and Winston. All rights reserved. Name Date Class SECTION 1 continued 7. Write net ionic equations that represent the following reactions: a. the ionization of HClO3 in water ϩ → ϩ ϩ Ϫ HClO3(aq) H2O(l ) H3O (aq) ClO3 (aq) b. NH3 functioning as an Arrhenius base ϩ → ϩ ϩ Ϫ NH3(aq) H2O(l ) ← NH4 (aq) OH (aq) 8.
    [Show full text]
  • Combining Sodium Bicarbonate and Lidocaine Injection
    Combining Sodium Bicarbonate and Lidocaine injection Tom Simpleman Consultant Pharmacist the FAWKS company http://dailymed.nlm.nih.gov/dailymed/lookup.cfm?setid=f9c826a7‐8f19‐4857‐b5be‐11dcafcfc7a9 Referenced information from National Institutes of Health DESCRIPTION: Sodium Bicarbonate Inj., 8.4% USP Neutralizing Additive Solution is a sterile, nonpyrogenic, solution of sodium bicarbonate (NaHCO3) in Water for Injection. It is added to an appropriate local anesthetic as a neutralizing agent immediately prior to administration. The solution contains no bacteriostat, antimicrobial agent or added buffer and is intended only for single-use. pH is adjusted with carbon dioxide. Per the USP monograph for Sodium Bicarbonate Inj., pH is between 7.0 and 8.5. Osmolar concentration is 2 mOsmol/mL (calc.). Sodium bicarbonate, 84 mg is equal to one milliequivalent each of Na+ and HCO3-. Sodium Bicarbonate, USP is chemically designated as NaHC03, a white crystalline powder soluble in water. Sodium bicarbonate in water dissociates to provide sodium (Na+) and bicarbonate (HCO3-) ions. Sodium (Na+) is the principal cation of the extracellular fluid and plays a large part in the therapy of fluid and electrolyte disturbances. Bicarbonate (HCO3-) is a normal constituent of body fluids and the normal plasma level ranges from 24 to 31 mEq/liter. Bicarbonate anion is considered “labile” since at a proper concentration of hydrogen ion (H+) it may be converted to carbonic acid (H2CO3) and thence to its volatile form, carbon dioxide (CO2) excreted by the lung. Normally a ratio of 1:20 (carbonic acid; bicarbonate) is present in the extracellular fluid. In a healthy adult with normal kidney function, practically all the glomerular filtered bicarbonate ion is reabsorbed; less than 1% is excreted in the urine.
    [Show full text]
  • Important Prescribing Information
    Important Prescribing Information Subject: Temporary importation of 8.4% Sodium Bicarbonate Injection to address drug shortage issues June 14, 2019 Dear Healthcare Professional, Due to the current critical shortage of Sodium Bicarbonate Injection, USP in the United States (US) market, Athenex Pharmaceutical Division, LLC (Athenex) is coordinating with the U.S. Food and Drug Administration (FDA) to increase the availability of Sodium Bicarbonate Injection. Athenex has initiated temporary importation of another manufacturer’s 8.4% Sodium Bicarbonate Injection (1 mEq/mL) into the U.S. market. This product is manufactured and marketed in Australia by Phebra Pty Ltd (Phebra). At this time, no other entity except Athenex Pharmaceutical Division, LLC is authorized by the FDA to import or distribute Phebra’s 8.4% Sodium Bicarbonate Injection, (1 mEq/mL), 10 mL vials, in the United States. FDA has not approved Phebra’s 8.4% Sodium Bicarbonate Injection but does not object to its importation into the United States. Effective immediately, and during this temporary period, Athenex will offer the following presentation of Sodium Bicarbonate Injection: Sodium Bicarbonate Injection, 8.4% (1mEq/mL), 10mL per vial, 10 vials per carton Ingredients: sodium bicarbonate, water for injection, disodium edetate and sodium hydroxide (pH adjustment) Marketing Authorization Number in Australia is: 131067 Phebra’s Sodium Bicarbonate Injection contains the same active ingredient, Sodium Bicarbonate, in the same strength and concentration, 8.4% (1 mEq/mL) as the U.S. registered Sodium Bicarbonate Injection, USP by Pfizer’s subsidiary, Hospira. However, it is important to note that Phebra’s Sodium Bicarbonate Injection (1 mEq/mL), is provided only in a Single Use 10 mL vials, whereas Hospira’s product is provided in 50 mL single-dose vials and syringes.
    [Show full text]
  • UNITED STATES PATENT OFFICE. ">Co
    UNITED STATES PATENT OFFICE. LEONHARD LEDERER, OF MUNICH, GERMANY. PROCESS OF PRE PARNG HAO D DERVATIVES OF ACET ONE. SPECIFICATION forming part of Letters Patent No. 643,144, dated February 13, 1900. Application filed August 10, 1897, Serial No. 647,759. (No specimens.) To all livhon, it nay conce77: iodacetone. Also if not kept dry it some Beit known that I, LEONHARDLEDERER, a times undergoes decomposition at an ordi citizen of the Kingdom of Bavaria, residing nary temperature, thereby evolving so much SO at Munich, Bavaria, Germany, have invented heat that vapor of iodin is set free. Alco a new and useful Process of Preparing the hol, ether, and most of the organic solvents IIalogen Derivatives of Acetone, of which the set free iodin from per-iod-acetone. With following is a specification. dilute soda-lye it forms iodoform in the cold. 55 It is well known that the halogens act read The action of iodin on acetone-dicarbonic. ily upon acetonedicarbonic acid. For in acid can be so regulated by definite diminu stance, bromin added to an aqueous solution tions of the quantity of iodin added as to re of acetonedicarbonic acid is immediately sult in lower stages of iodin combination with taken up. An aqueous solution of acetonedi acetone. With regard to its behavior toward carbonic acid decomposed with an alcoholic alcohol and ether the penta-iod derivative is iodin solution takes up quickly the color of in close relation with the periodacetone. On the latter without visible reaction. If, how the addition of dilute soda-lye it is trans ever, this mixture be gently Warmed, reac formed into iodoform even in the cold, but tion takes place, evolving carbonic acid gas; not with the soda solution.
    [Show full text]
  • Structure and Functioning of the Acid–Base System in the Baltic Sea
    Earth Syst. Dynam., 8, 1107–1120, 2017 https://doi.org/10.5194/esd-8-1107-2017 © Author(s) 2017. This work is distributed under the Creative Commons Attribution 3.0 License. Structure and functioning of the acid–base system in the Baltic Sea Karol Kulinski´ 1, Bernd Schneider2, Beata Szymczycha1, and Marcin Stokowski1 1Institute of Oceanology, Polish Academy of Sciences, IO PAN, ul. Powstanców´ Warszawy 55, 81-712 Sopot, Poland 2Leibniz Institute for Baltic Sea Research Warnemünde, IOW, Seestrasse 15, 18119 Rostock, Germany Correspondence: Karol Kulinski´ ([email protected]) Received: 6 April 2017 – Discussion started: 12 April 2017 Revised: 21 October 2017 – Accepted: 6 November 2017 – Published: 11 December 2017 Abstract. The marine acid–base system is relatively well understood for oceanic waters. Its structure and func- tioning is less obvious for the coastal and shelf seas due to a number of regionally specific anomalies. In this review article we collect and integrate existing knowledge of the acid–base system in the Baltic Sea. Hydro- graphical and biogeochemical characteristics of the Baltic Sea, as manifested in horizontal and vertical salinity gradients, permanent stratification of the water column, eutrophication, high organic-matter concentrations and high anthropogenic pressure, make the acid–base system complex. In this study, we summarize the general knowledge of the marine acid–base system as well as describe the peculiarities identified and reported for the Baltic Sea specifically. In this context we discuss issues such as dissociation constants in brackish water, differ- ent chemical alkalinity models including contributions by organic acid–base systems, long-term changes in total alkalinity, anomalies of borate alkalinity, and the acid–base effects of biomass production and mineralization.
    [Show full text]
  • Ph Buffers in the Blood
    pH Buffers in the Blood Authors: Rachel Casiday and Regina Frey Department of Chemistry, Washington University St. Louis, MO 63130 For information or comments on this tutorial, please contact R. Frey at [email protected]. Please click here for a pdf version of this tutorial. Key Concepts: Exercise and how it affects the body Acid-base equilibria and equilibrium constants How buffering works Quantitative: Equilibrium Constants Qualitative: Le Châtelier's Principle Le Châtelier's Principle Direction of Equilibrium Shifts Application to Blood pH How Does Exercise Affect the Body? Many people today are interested in exercise as a way of improving their health and physical abilities. But there is also concern that too much exercise, or exercise that is not appropriate for certain individuals, may actually do more harm than good. Exercise has many short-term (acute) and long-term effects that the body must be capable of handling for the exercise to be beneficial. Some of the major acute effects of exercising are shown in Figure 1. When we exercise, our heart rate, systolic blood pressure, and cardiac output (the amount of blood pumped per heart beat) all increase. Blood flow to the heart, the muscles, and the skin increase. The body's metabolism becomes more active, producing CO and H+ in the muscles. We breathe faster and deeper to supply the oxygen 2 required by this increased metabolism. Eventually, with strenuous exercise, our body's metabolism exceeds the oxygen supply and begins to use alternate biochemical processes that do not require oxygen. These processes generate lactic acid, which enters the blood stream.
    [Show full text]
  • Carbon Species of the Lithosphere and Hydrosphere: the Carbonic Acid System1
    Experiment 18B SC151 10/07/10 CARBON SPECIES OF THE LITHOSPHERE AND HYDROSPHERE: 1 THE CARBONIC ACID SYSTEM MATERIALS: pH meter (2); magnetic stirrer and stirbar (2); standardization buffers (pH=4, 7 and 10); 50 mL buret (2); 400 mL beaker (3); 100 mL beaker (2); 100 mL graduated cylinder; filter funnel and filter paper; anhydrous Na2CO3; saturated solution of MgCO3; 0.036 M H2SO4; 0.0072 M H2SO4. PURPOSE: The purpose of this experiment is to introduce the use of the pH meter and to identify important features in the titration curves of weak acids and bases. LEARNING OBJECTIVES: By the end of this experiment, the student should be able to demonstrate the following proficiencies: 1. Standardize and use a pH meter. 2. Perform a pH titration. 3. Identify the dominant chemical species at various points in a titration curve. 4. Obtain values of pKa for weak acids from pH titration data. DISCUSSION Every carbon atom in your body has been used in countless other molecules since the beginning of time, as CO2 in the air you breathe, as carbohydrates in the food you eat, as bicarbonate “fixed” by sea life, or as carbonate salts in the rocks and soil you walk on. The Carbon Cycle is a complex series of processes which describes how carbon atoms circulate among these realms of atmosphere, biosphere, hydrosphere and lithosphere. By far, the greatest store of carbon atoms on earth can be found in marine sediments and sedimentary rocks (~8 x 1016 metric tons), with the ocean providing a distant second store (~4x1013 metric tons).
    [Show full text]
  • Mineral Carbonation and Industrial Uses of Carbon Dioxide 319 7
    Chapter 7: Mineral carbonation and industrial uses of carbon dioxide 319 7 Mineral carbonation and industrial uses of carbon dioxide Coordinating Lead Author Marco Mazzotti (Italy and Switzerland) Lead Authors Juan Carlos Abanades (Spain), Rodney Allam (United Kingdom), Klaus S. Lackner (United States), Francis Meunier (France), Edward Rubin (United States), Juan Carlos Sanchez (Venezuela), Katsunori Yogo (Japan), Ron Zevenhoven (Netherlands and Finland) Review Editors Baldur Eliasson (Switzerland), R.T.M. Sutamihardja (Indonesia) 320 IPCC Special Report on Carbon dioxide Capture and Storage Contents EXECUTIVE SUMMARY 321 7.3 Industrial uses of carbon dioxide and its emission reduction potential 330 7.1 Introduction 322 7.3.1 Introduction 330 7.3.2 Present industrial uses of carbon dioxide 332 7.2 Mineral carbonation 322 7.3.3 New processes for CO2 abatement 332 7.2.1 Definitions, system boundaries and motivation 322 7.3.4 Assessment of the mitigation potential of CO2 7.2.2 Chemistry of mineral carbonation 323 utilization 333 7.2.3 Sources of metal oxides 324 7.3.5 Future scope 334 7.2.4 Processing 324 7.2.5 Product handling and disposal 328 References 335 7.2.6 Environmental impact 328 7.2.7 Life Cycle Assessment and costs 329 7.2.8 Future scope 330 Chapter 7: Mineral carbonation and industrial uses of carbon dioxide 321 EXECUTIVE SUMMARY This Chapter describes two rather different options for carbon and recycled using external energy sources. The resulting dioxide (CO2) storage: (i) the fixation of CO2 in the form of carbonated solids must be stored at an environmentally suitable inorganic carbonates, also known as ‘mineral carbonation’ or location.
    [Show full text]
  • Ph Regulation During Exercise Acid-Base Equilibria Experiment
    Blood, Sweat, and Buffers: pH Regulation During Exercise Acid-Base Equilibria Experiment Authors: Rachel Casiday and Regina Frey Revised by: C. Markham, A. Manglik, K. Castillo, K. Mao, and R. Frey Department of Chemistry, Washington University St. Louis, MO 63130 For information or comments on this tutorial, please contact Kit Mao at [email protected]. Key Concepts: • Exercise and how it affects the body • Acid-base equilibria and equilibrium constants • How buffering works Equilibrium Constants Henderson-Hasselbalch Equation Direction of Equilibrium Shifts Application to Blood pH Related Tutorials: • Hemoglobin and the Heme Group: Metal Complexes in the Blood for Oxygen Transport • Iron Use and Storage in the Body: Ferritin and Molecular Representations • Maintaining the Body’s Chemistry: Dialysis in the Kidneys How Does Exercise Affect the Body? Many people today are interested in exercise as a way of improving their health and physical abilities. When we exercise, our heart rate, systolic blood pressure, and cardiac output (the amount of blood pumped per heart beat) all increase. Blood flow to the heart, the muscles, and the skin + increase. The body's metabolism becomes more active, producing CO2 and H in the muscles. We breathe faster and deeper to supply the oxygen required by this increased metabolism. With strenuous exercise, our body's metabolism exceeds the oxygen supply and begins to use alternate biochemical processes that do not require oxygen. These processes generate lactic acid, which enters the blood stream. As we develop a long-term habit of exercise, our cardiac output and lung capacity increase, even when we are at rest, so that we can exercise longer and harder than before.
    [Show full text]
  • Ph – Carbonate Equilibrium and Applications to Manufacture of Still Water
    Carbonate Chemistry Applied to the Beverage Production of Still Water By Phillip L. Hayden, Ph.D., P.E. True North Thinking, LLC 591 Congress Park Drive Dayton, OH 45459 The chemistry of the carbonate equilibrium, including carbon dioxide (CO2), directly affects the beverage production of still water, which has strict pH and alkalinity standards. CO2 (g) will pass through a Reverse Osmosis (RO) membrane, which is commonly used in still water production, and end up in the final water. Unless the CO2 is removed, adjusting the final pH to specifications will result in high alkalinity concentrations in excess of the specifications. The purpose of this paper is to define the carbonate chemistry, present various treatment options and the impact of CO2 (gas) on final still water quality. 1.0 REVIEW Most ground waters have high levels of hardness consisting of calcium and magnesium ions and alkalinity, which are the carbonate ions. These waters, when removed from the ground, increase in temperature and become oversaturated with respect to precipitation of calcium carbonate. As a result, calcium carbonate scale forms on pipes, valves, heating coils and process equipment. High levels of calcium and magnesium also impact the sensory qualities of carbonated soft drink products (CSD). In groundwater’s originating from limestone aquifers, the hardness ions calcium and magnesium are normally accompanied with carbonate alkalinity. The carbonate equilibrium, which includes free CO2 or carbonic acid, bicarbonate ions and carbonate ions, is highly pH dependent. The CO2 – bicarbonate equilibrium exists in the pH range of 4.3 to 8.3 and the bicarbonate – carbonate equilibrium dominating at pH 8.3 – 12.3.
    [Show full text]
  • Model Carbonate Blood Buffer Introduction SCIENTIFIC the Ph Level in Blood Must Be Maintained Within Extremely Narrow Limits
    Model Carbonate Blood Buffer Introduction SCIENTIFIC The pH level in blood must be maintained within extremely narrow limits. What is the composition of the major buffer in blood? Concepts • Buffer • Conjugate base • Weak acid Background All buffers contain a mixture of a weak acid (HA) and its conjugate base (A–). The buffer components HA and A– are related to each other by means of the following chemical reaction (Equation 1). → – + HA + H2O ← A + H3O Equation 1 weak acid conjugate base Buffers control pH because the two buffer components react with and neutralize either strong acid or strong base that might be added. The weak acid HA reacts with any strong base, such as sodium hydroxide (NaOH), to give water and the conjugate base A– (Equation 2). The conjugate base A– reacts with any strong acid, such as hydrochloric acid (HCl), to give its acid partner HA (Equation 3). → + – HA + NaOH ← Na + A + H2O Equation 2 A– + HCl ←→ HA + Cl– Equation 3 These neutralization reactions can be visualized as a cyclic process (Figure 1). Buffer activity will continue as long as both components are present. The pH range in which a buffer system will be effective is called its buffer range. The buffer range is 2 pH units centered around the pKa value of the weak acid. – The major buffer in blood is composed of carbonic acid (H2CO3) and its conjugate base, bicarbonate ion (HCO3 ) (Equation 4). A carbonic acid–bicarbonate buffer has a buffer range of pH 5.4–7.4. The normal pH of blood (7.2) is at the upper limit of the effective range for the carbonic acid–bicarbonate buffer system.
    [Show full text]